Final answer:
The electron configuration for Fe2+ is 1s2 2s2 2p6 3s2 3p6 3d6, with the loss of two 4s electrons, while the electron configuration for P3- is 1s2 2s2 2p6 3s2 3p6, with the filling of the 3p orbital to mimic the noble gas argon.
Step-by-step explanation:
The question pertains to predicting the electron configurations for iron (Fe) in its +2 oxidation state (ion) and for phosphorus (P) in its -3 oxidation state (anion). The electron configuration of an ion helps to explain the chemical properties it will exhibit, including bonding and reactivity.
For Fe2+, the electron configuration would be 1s22s22p63s23p63d6. When iron forms Fe2+, it loses two electrons from the 4s orbital, which are the highest energy electrons. The 4s electrons are lost before the 3d electrons due to their higher energy level in the ionized state.
For P3-, the electron configuration would be 1s22s22p63s23p6. In gaining three electrons to form a P3- anion, phosphorus achieves the electron configuration of the noble gas argon, as the extra electrons fill the 3p orbital.